(6) A mixture of 40.0 g of oxygen and 40.0 g of helium has a total pressure of 0.900 atm.
What is the partial pressure of each gas?

The partial pressure of each gas are:

1. The partial pressure of oxygen is 0.1 atm.

2. The partial pressure of helium is 0.8 atm.

We'll begin by calculating the number of mole of each gas:

Mass = 40 g

Molar mass = 32 g/mol

Mole = mass / molar mass

Mole of Oxygen = 40 / 32

Mass = 40 g

Molar mass = 4 g/mol

Mole = mass / molar mass

Mole of Helium = 40 / 4

Mole of Oxygen = 1.25 mole

Mole of Helium = 10 moled

Total mole = 1.25 + 10

Mole of Oxygen = 1.25 mole

Total mole = 11.25 moles

Mole fraction = mole / total mole

Mole fraction of Oxygen = 1.25 / 11.25

1. Determination of the partial pressure of oxygen

Mole fraction of Oxygen = 0.111

Total pressure = 0.9 atm

Partial pressure = mole fraction × total pressure

Partial pressure of Oxygen = 0.111 × 0.9

2. Determination of the partial pressure of Helium

Partial pressure of Oxygen = 0.1 atm

Total pressure = 0.9 atm

Partial pressure of Helium = Total pressure – Partial pressure of Oxygen

Partial pressure of Helium = 0.9 – 0.1

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Partial pressure of oxygen   atm

Partial pressure of Helium   atm

Explanation:

We will first find the number of moles of each gas

The molar mass of oxygen is grams per mole

The molar mass of helium is grams per mole

The number of moles of oxygen in the solution

The number of moles of helium in the solution

The number of moles of oxygen in the solution

Total number of moles in the solution is equal to

Partial pressure of oxygen

atm

atm

Partial pressure of Helium

atm

atm

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.